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Chemistry / Chemistry 11 / Chapter 23 / Problem 14P

Chemistry | 11th Edition | ISBN: 9780073402680 | Authors: Raymond Chang

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Give the oxidation numbers of the metals in the

Chapter 23, Problem 14P

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QUESTION:

Give the oxidation numbers of the metals in the following species: (a) \(\mathrm{Na}_{2} \mathrm{MoO}_{4}\), (b) \(\mathrm{MgWO}_{4}\), (c) \(\mathrm{Fe}(\mathrm{CO})_{5}\).

Questions & Answers

QUESTION:

Give the oxidation numbers of the metals in the following species: (a) \(\mathrm{Na}_{2} \mathrm{MoO}_{4}\), (b) \(\mathrm{MgWO}_{4}\), (c) \(\mathrm{Fe}(\mathrm{CO})_{5}\).

ANSWER:

Step 1 of 4

Oxidation number:

The number of electrons an atom or ion has either gained or lost to the neutral atom is known as the oxidation number or state of the atom or ion.

Rules for assigning oxidation numbers:

$\bullet{}$ All elements in their free state have an oxidation of zero.

$\bullet{}$ is except in metal hydrides , where it is .

$\bullet{}$ is except in peroxides, where it is and in , where it is .

$\bullet{}$ All metallic elements in an ionic compound have a positive oxidation number.

$\bullet{}$ The sum of all oxidation numbers of atoms or ions in a neutral compound is zero.

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